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Chem Flashcards

1
Q

what is an atom?

A

the most basic complete unit of an element

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2
Q

Element

A

Pure Substances that cannot be broken into simpler substances

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3
Q

What are the three fundamental particles/ subatomic particles of an atom?

A

proton, neutrons, and electrons

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4
Q

Valence Electrons

A

the electrons in the outer most shells that can bond

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5
Q

The elements in the first period have how many shells

A

1 shell - s
Period or row 2 has subsell s and subshell p

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6
Q

The elements in the 7th period have how many sub shells

A

7

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7
Q

Atomic number

A

number of protons in the nucleus of an atom

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8
Q

atomic mass

A

the sum of the masses of protons and neutrons in one atom of an element

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9
Q

what are electrons and where are they located?

A

Electrons are negatively charged subatomic particles that move around the center of the atom in regions known as orbitals

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10
Q

how many electrons can each orbital hold

A

2 electons

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11
Q

Orbitals group together to make up a …

A

shell

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12
Q

What are the subshells labeled as

A

S,P,D, F with s being closest to the nucleus

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13
Q

What is the most stable configuration for valence electrons

A

atoms in their most stable state when their valence shells are filled.

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14
Q

What are the two exceptions to the 8 valence electron rule

A

hydrogen and helium

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15
Q

What two subatomic particles are in the nucleus

A

neutrons and protons

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16
Q

Atomic mass units

A

amu

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17
Q

why are electrons not included in the atomic mass

A

they have such a slight mass that they are not inlcuded

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18
Q

how does atomic number ( protons) change across the periodic table

A

the atomic number increases left to right and

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19
Q

Maximum Number of Electrons for an S orbital

A

2

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20
Q

Maximum Number of Electrons for an P orbital

A

p = 6

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21
Q

Maximum Number of Electrons for an d orbital

A

d = 10

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22
Q

Maximum Number of Electrons for an f orbital

A

f = 14

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23
Q

Orbitals in period 1, 2, 3, 4

A

1 = s
2 - s,p
3 = s, p,d
4 -= s, p,d, f

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24
Q

HOW ARE COLUMNS Arranged

A

each column ( group) contains elements that have similar chemical and physical properties

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25
Q

Isotopes

A

Atoms of the same element that have different numbers of neutrons but the same number of protons and electrons.

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26
Q

Ion

A

a positively or negatively charged atom or molecule

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27
Q

cation

A

positively charged ion

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28
Q

anion

A

negatively charged ion

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29
Q

typically metals that are on the left side of the periodic table become what type of ion

A

lose electrons when they form ions

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30
Q

elements in the upper right of the periodic table, the nonmetals become what type of ion

A

gain electrons to form anions

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31
Q

Reactions of metals and nonmetals form compounds with what type of bonds

A

ionic bonds

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32
Q

ionic bonds

A

the bond between two oppositely charged ions
the ionic bond occurs when the metal transfer electrons to the nonmetal

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33
Q

reactions between nonmetals result in what type of bond

A

covalent bond - sharing of electrons

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34
Q

Physical Properties of Substances

A

observable characteristics that change without modifying the identity of the substance.

ex. state of matter

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35
Q

Three common states of matter

A

solid, liquid, gas

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36
Q

Intensive Properties

A

physical properties that are independent on the amount of substance present
ex: density, color, conductivity

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37
Q

extensive properites

A

Physical properties that are Dependent on the amount of substance present
ex: length, volume, mass

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38
Q

Mass

A

a measurement of inertia, commonly considered the amount of material contained by an object and causing it to have weight in a gravitational field

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39
Q

Volume

A

the amount of space something takes up

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40
Q

Length

A

Measurement of distance from end to end

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41
Q

Can volume and mass independently be used to identify and substance

A

No, density ( mass/ volume) is an intensive property that is constant for each substance and can be used for identification

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42
Q

density

A

Mass/ Volume - an intensive property

denser substances will sink below less dense substances

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43
Q

Molecules above absolute are

A

in constant motion

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44
Q

0 Kelvin = X Celcius

A

-273 celcius

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45
Q

Molecule

A

an arrangement of two or more atoms bonded together

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46
Q

How does heat change an atoms motions

A

the amount of movement within a molecule ( and atom) increases in response to thermal energy ( heat)

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47
Q

Intermolecular forces

A

molecule to molecule bonding

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48
Q

What is the fourth phase of matter

A

plasma

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49
Q

plasma

A

clear pale yellow components of blood that caries red blood cells, white bc, and platelets throughout the body.

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50
Q

what are molecules in constant motion?

A

bc their atoms are in constant motion - making and breaking bonds

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51
Q

temperature

A

a measure of the average energy of the molecules within a substance - aka the hotness or coldness of a substance

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52
Q

are heat and temperature the same?

A

no

53
Q

heat

A

a measured unit of calories or joules
heat can be thought of as energy that is generated by or applied to a substance or system

54
Q

The amount of energy needed to change the temperature of one gram of a molecule by 1 degrees C is called what

A

its specific heat of capacity

55
Q

The phase of a substance depends on two conditons:

A

temperature and pressure

56
Q

how does increasing temp and increasing pressure affect movement of particles

A

increasing temp as the tendency to move particles apart
increasing pressure has a tendency to move particles of matter together

57
Q

Liquid state

A

definite volume but not definite shape

57
Q

lower temperature of a substance correlates to

A

less IMF movement

58
Q

Evaporation

A

liquid to gas

59
Q

gas

A

a state of matter composed of molecules in constant random motion
no definite volume or shape - it is highly compressible

60
Q

condensation

A

gas to liquid

61
Q
A
61
Q

triple point

A

the temperature and pressure at which solid, liquid, and gas phases of a pure substance coexist

62
Q

deposition

A

the transition of substance from gas to solid

63
Q

sublimation

A

the transition of a substance from solid to gas

64
Q

critical point

A

the temperature above which a substance coexists in both its liquid and gas states

65
Q

Chemical Reaction

A

a process in which one bonding arrangement among atoms is exchanged for a different bonding arrangement

66
Q

Molecule

A

any arrangement of two or more atoms bonded together

67
Q

Valence electrons

A

The electrons in the outermost shell of an atom have the highest energy and are easily transferred or shared with other atoms

68
Q

Elements in the same group (vertical column) on the periodic table have

A

the same number of valence electrons in the same type of subshell ( s,p,d,f)

69
Q

ionization trend

A

generally speaking, the left side of the periodic table has elements with low ionization energies - moving to the upper right have high ionization energies and electronegativities so they tend to gain electrons in chemical reactions

70
Q

ionic bond

A

the bond between two oppositely charged ions

71
Q

covalent bond

A

the result of two or more atoms sharing electrons so both atoms involved becomes more stable

72
Q

typically, an atom having fewer than four valence shell electrons

A

will lose its electrons to an atom with more than four valence shell electrons

73
Q

Solution

A

a homogeneous mixture of two or more substances whose components are uniformly distributed on a microscopic scale

74
Q

compound

A

a substance made of two or more elements

75
Q

reactants

A

in chemical equation, the substances on the left side of the equation; the starting materials in a chemical reaction

76
Q

products

A

the substances that are formed in a chemical reaction

77
Q

metal

A

a substance that is a good conductor of electricity and heat, forms cations by loss of electrons, and yields basic oxides and hydroxides

78
Q

a mole

A

a unit - 1 mol = 6.022 * 10^23 particles

79
Q

activation energy

A

the minimum energy required to initiate a chemical rxn

80
Q

pH

A

the measure of acidity or alkalinity

81
Q

Catalyst

A

a substance that increases the rate of a chemical reaction without undergoing

82
Q

endothermic rxn

A

involving absorption of heat

83
Q

exothermic rxn

A

involving the release of heat

84
Q

Increasing the concentration of reactants

A

increases the probability that reactants will come in contact with each other

85
Q

if products are withdrawn from the reaction as they form

A

the rate of production formation increases

86
Q

increase in pressure will

A

increase the number of interactions between reactant molecules and thus, increase the rate of reaction

87
Q

activation energy

A

the minimum energy required to initiate a chemical reaction

88
Q

the smaller the activation barrier the

A

faster the rate of the reaction

89
Q

the most important biological catalysts are

A

enzymes

90
Q

once equilibrium is reached

A

the rates of the forward and reverse reactions are equal. there is no change in the concentration of reactants or products

91
Q

what causes change of direction of a reaction?

A

change in concentration can
decreasing the concentration shifts the reaction to the left and increasing the concentration of a reactant shift the reaction right.

think lungs at co2 - decreasing the concentration by exhaling drives the reaction to form more of it

92
Q

Le Chatelier’s principle

A

when a chemical reaction at equilibrium is perturbed, it responds by going in the direction that restores the equilibrium

changing [pressure and temperature can also perturb a reaction that is at equilibirum

93
Q

If the reaction is exothermic, raising the temperature would

A

shift the reaction to the left

94
Q

Increasing the temperature of an endothermic reaction will

A

increase the rate of reaction

95
Q

CO2 is _________ in respiring tissue, but _________ in the lungs

A

Co2 is formed in respiring tissue and expelled via exhalation in the lungs; therefore, CO2 concentration is high in respiring tissue and low in the lungs - high Co2 favors the forward direction, and low Co2 favors the reverse

96
Q

Solutions

A

are homogenous mixtures of two or more substances whose components are uniformly distributed on a microscopic scale

97
Q

Polar Bonds

A

is a covalent bond in which the atoms have an unequal attraction for electrons, and so the sharing is unequal.

98
Q

Nonpolar covalent Bonds

A

is a covalent bond in which the bonding electrons are shared equally between the two atoms. In a nonpolar covalent bond, the distribution of electrical charge is balanced between two atoms

99
Q

Hydrogen Bonding

A

a weak bond formed between the partial negative region and partial positive region
( ex. neg of oxy and pos of hydrogen in water)

100
Q

Water is the universal

A

solvent

101
Q

Adhesion

A

the tendency of dissimilar particles or surfaces to cling to one another

102
Q

Cohesion

A

stick to itself

103
Q

cohesion creates

A

surface tension
and with adhesion it helps creates capillary action that moves water up the plant xylem

104
Q

water has a ( high/low) specific heat capacity

A

high specific heat capacity

105
Q

why is water denser as liquid than solid

A

due to hydrogen bonds liquid water is more dense than solid water.
ice floats on water because more hydrogen bonds form between water with lower Kinetic energy

in other words - for the same mass of water, solid water takes up more volume and therefore it is less dense than liquid water

106
Q

solution

A

when one substance dissolves into another where the solvent is the substance that dissolves a solute

107
Q

what is in larger proportion the solvent or the solute

A

the solvent constitutes a greater proportion of the solution than the solute so the solution exists as the same phase as the solvent

if solute = solid, solvent = liquid … the solution = liquid

108
Q

hydrophilic

A

water-loving

109
Q

hydrophobic

A

water fearing

110
Q

solubility of most substances depends strongly on

A

the temperature, and in the case of gases, the pressure.

111
Q

the solubility of most solids and liquids _______ as temp increases

A

increases

112
Q

the solubility of gas ________ as temp increases

A

Decreases

113
Q

saturated solution

A

a solution containing the maximum possible amount of solute

114
Q

supersaturated solutions

A

contain more dissolved solutes than saturated solutions bc the solute is dissolved in the solvent at higher temperatures

115
Q

Molarity

A

moles of solute / liter of solution ( mol/L)

116
Q

Mole fraction

A

Moles of solute/ total moles present ( mol/mol)

117
Q

Molality

A

Moles of solute / kg of solvent ( mol/kg)

118
Q

Mass percentage

A

( mass of solute (g)/ mass of solution (g)) * 100

119
Q

parts per thousand (ppt)

A

= g solute / kg solution

120
Q

parts per million (ppm)

A

mg solute / kg solution

units of ppm or ppb are used to express very low concentrations

121
Q

parts per billion (ppb)

A

ug solute / kg solution

units of ppm or ppb are used to express very low concentrations

122
Q

Ionic bond

A

transfer due to the attraction of oppositely charged ions that resulted from the electron transfer

123
Q

dissolution of ionic bonds result in ..

A

solvent molecules surrounding ions ( rather than uncharged particles)
example - diffusion

124
Q

ions are unable to pass through the lipid bilayer of a cell membrane so there movement depends on

A

specialized ion channels on the membrane of cells which use active transport

125
Q

active transport in cells

A

movement across a cell membrane that travels against the concentration gradient and thus requires energy

126
Q

osmosis

A

the diffusion of water across a semipermeable membrane such as a cell membrane

( water like ions does not move easily though the cell membrane’s lipid bilayer. it moves though pores ( made of aquaporin protein) by way of osmosis which does not require energy use

127
Q
A

Teas (4 decks)

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